Question

Calculate the pressure, in atmospheres, of 2.43 moles of helium gas in a 10.0- L container at 27 ∘C .

Answer 1

To answer this question, we have to use the ideal gas law:

`PV=nRT`

Where P is pressure, V is volume, n is the number of moles, R is the constant of ideal gases (0.082atmL/molK) and T is the temperature (in Kelvin degrees).

Convert the given temperature to Kelvin degrees:

`T=27+273.15=300.15`

Solve the equation for P and replace for the given values:

`\begin{gathered} P=(nRT)/(V) \\ P=(2.43mol\cdot0.082atmL/molK\cdot300.15K)/(10.0L) \\ P=5.98atm \end{gathered}`

It means that the pressure of helium is 5.98atm.